sodium metal reacts with water to produce hydrogen gas according to the followin
ID: 704697 • Letter: S
Question
sodium metal reacts with water to produce hydrogen gas according to the following equatuion: 2Na(s) + 2H2O(l) -> 2NaOH(aq) + H2 (g). in an experiment. the hydrogen gas is collected over water in a vessel where the total pressure is 745 torr and the temperature is 20 c, at which temperature the vapor pressure of water is 17.5 torr. under these conditions, what it the partial pressure of hydrogen? if the wet hydrogen gas formed occupied a volume of 8.04 L, what number of moles of hydrogen is formed?
Explanation / Answer
2Na(s) + 2H2O(l) -> 2NaOH(aq) + H2 (g).
the total pressure is 745 torr
the vapor pressure of water is 17.5 torr
the partial pressure of hydrogen = the total pressure - the vapor pressure of water
= 745-17.5 = 727.5 torr
PH2 = 727.5 torr = 727.5/760 = 0.96atm
V = 8.04 L
T = 20+273 = 293K
PV = nRT
n = PV/RT
= 0.96*8.04/0.0821*293 = 0.32 moles
The number of moles of hydrogen is 0.32 moles >>>>answer
Related Questions
Navigate
Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.